The sublevel designation, the allowable ml values, and the number of orbitals are,
For ,n = 2, l = 0 ⇒ sublevel s, ⇒ ml = 0, number of orbitals = 1
The rules for electron quantum numbers are:
1. Shell number, 1 ≤ n,
2. Subshell number, 0 ≤ l ≤ n − 1, from s, p, d, f, g, h...
3. Orbital energy shift, -l ≤ ml ≤ l
4. Spin, either -1/2 or +1/2
-l ≤ ml ≤ l ⇒ ml = 0
number of orbitals = 1
Where a specific electron can be found within a nucleus is described using quantum numbers. Each electron in an atom can be defined by one of four quantum numbers. N, L, M 1, and M S Each number has a range of possible values determined by a set of rules.
The collection of numbers known as quantum numbers are used to express the location and energy of an electron in an atom. The main, azimuthal, magnetic, and spin types of quantum numbers are the four categories. The values of the conserved quantities in a quantum system are represented by quantum numbers.
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